holding a lit match to paper
no
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For example any chemical reaction need an activation energy.
Activation energy is the minimum amount of energy required for a chemical reaction to occur. For example, when lighting a match, the activation energy provided by the friction between the match and the striking surface initiates the combustion reaction.
No, heating a flask on a hot plate is not an example of activation energy beginning to react. Activation energy refers to the minimum amount of energy required for a chemical reaction to occur, and it is not related to heating a flask. Heating a flask on a hot plate simply refers to the process of applying heat to the flask, which can facilitate a reaction by increasing the temperature and providing the necessary energy for the reaction to proceed.
An exergonic reaction is activation energy (or energy of activation). An endergonic reaction is essentially the opposite of an exergonic reaction.
Activation energy is the minimum amount of energy required for a chemical reaction to occur. In inorganic chemistry, activation energy determines the rate at which reactions proceed. Higher activation energy results in slower reactions, while lower activation energy results in faster reactions. By understanding activation energy, chemists can optimize reaction conditions and develop more efficient processes.
The minimum amount of energy needed to start a chemical reaction is called the activation energy. It is the energy required to break the bonds in reactant molecules and initiate the reaction. Once this energy barrier is overcome, the reaction proceeds without additional energy input.
That is called the activation energy or energy of activation (Ea).
The energy needed to get a reaction started is called activation energy.
Activation energy is the energy required by a reaction for the reaction to occur. The catalyst lowers the activation energy, making it easier for the reaction to happen.Improvement:A catalyst don't lowers the activation energy. A catalyst creates a alternative route (*) for the same reaction with a lower activation energy.* = as a result of the interaction of the reagents with the catalyst.
Activation energy describes the energy that is required to get chemical reactions started.